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(C) The osmotic pressure $(\pi)$ is given by the formula $\pi = iCRT$,where $i$ is the van't Hoff factor,$C$ is the molar concentration,$R$ is the gas

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$M/10$ $BaCl_2$

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(C) The osmotic pressure $(\pi)$ is given by the formula $\pi = iCRT$,where $i$ is the van't Hoff factor,$C$ is the molar concentration,$R$ is the gas constant,and $T$ is the temperature.Since $C$,$R$,and $T$ are constant for all given solutions,the osmotic pressure depends directly on the van't Hoff factor $(i)$.For $NaCl$,$i = 2$ (dissociates into $Na^+$ and $Cl^-$).For Urea,$i = 1$ (non-electrolyte).For $BaCl_2$,$i = 3$ (dissociates into $Ba^{2+}$ and $2Cl^-$).For Glucose,$i = 1$ (non-electrolyte).Since $BaCl_2$ has the highest van't Hoff factor $(i = 3)$,it will have the maximum osmotic pressure.

Which of the following solutions has the maximum osmotic pressure?

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